Question

What mass of c2h6 is necessary to produce 280.0 g co2 in the following reaction?

1. What is the molar mass of C₂H₆ (ethylene)?
a. 26 g/molb. 28 g/molc. 30 g/mold. 32 g/mol
2. How many moles of CO₂ are produced in the reaction for every mole of C₂H₆?
a. 1 molb. 2 molc. 3 mold. 4 mol
3. If the reaction produces 280.0 g of CO₂, how many grams of C₂H₆ were used?
a. 140 gb. 160 gc. 180 gd. 200 g

Answer 1

1. The molar mass of C₂H₆ is c. 30 g/mol

2. moles of CO₂ are produced in the reaction is b. 2 mol

3. grams of C₂H₆ were used in the reaction c. 180 g

How to find the number of moles

Molar Mass of C₂H₆

= 2 * atomic mass of C + 6 * atomic mass of H

= 2 * 12 + 6 * 1

= 24 + 6

= 30

So the correct answer is:

c. 30 g/mol

Moles of CO₂ produced per mole of C₂H₆:

The balanced chemical equation for the combustion of C₂H₆ is:

C₂H₆ + 7/2 O₂ → 2 CO₂ + 3 H₂O

From the balanced equation, we see that 1 mole of C₂H₆ produces 2 moles of CO₂.

So, the correct answer is:

b. 2 mol

Grams of C₂H₆ used to produce 280.0 g of CO₂:

Using the information from the previous parts, we know that 1 mole of C₂H₆ produces 2 moles of CO₂.

Given that 280.0 g of CO₂ is produced,

moles of CO₂ = mass of CO₂ / molar mass of CO₂

= 280 / 44

Using proportion

1 mole ⇒ 2 moles

? ⇒ 280/44

? = 280/44 * 1/2 = 3.18 moles

Molar Mass of C₂H₆ = 30

amount in grams = 30 * 3 = 180 g

So the correct answer is:

c. 180 g